Question

For the reversible, one-step reaction A+B<---->C+D, the forward rate constant is 52.4 /mol*h and the rate constant for the reverse reaction is 32.1 L/mol*h. The activation energy was found to be 35.2 kJ/mol for the forward reaction and 44.0 kJ.mol for the reverse reaction.

a) What is the equilibrium constant for the reaction?

b) is the reaction exothermic or endothermic?

c) What will be the effect of raising the temperature on the rate constants and the equilibrium constant?

Answer 1

Answer:

—-—1———————-s

Answer 2

• The equilibrium constant = 1.63

• The reaction is an exothermic reaction

• The effect of increased temperature is that the quantity of products would decrease.

Calculation of equilibrium constant

The rate constant for the forward reaction = 52.4/mol*h

The rate constant for the reverse reaction =32.1 L/mol*h.

Equilibrium constant:

(K) = kf/kb

K = 52.4/32.1

K= 1.63

• The reaction is an exothermic reaction because activation energy of forward reaction (35.2 kJ/mol) is less than the activation energy of the backward reaction (44.0 kJ.mol).

• The effect of of increased temperature is that the quantity of products would decrease.

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